Magnesium-substituted hydroxypatites

ABSTRACT

A stable, phase-pure magnesium-substituted crystalline hydroxyapatite containing from about 2.0 to about 29 wt % magnesium, wherein at least 75 wt % of the magnesium content is substituted for calcium ions in the hydroxyapatite lattice structure.

CROSS REFERENCE TO RELATED APPLICATION

This application is a Divisional of U.S. patent application Ser. No.09/800,127 (pending) which was filed on Mar. 6, 2001 with the UnitedStates Patent and Trademark Office, the disclosure of which isincorporated herein by reference.

BACKGROUND OF THE INVENTION

The present invention relates to methods for magnesium substitution ofcrystalline hydroxyapatites that provide heretofore unobtained levels ofmagnesium incorporation into the hydroxyapatite lattice structure. Thepresent invention also relates to phase-pure magnesium-substitutedcrystalline hydroxyapatites obtained thereby.

Hydroxyapatite (HAp, chemical formula Ca₁₀(PO₄)₆(OH)₂) has attracted theattention of researchers over the past thirty years as an implantmaterial because of its excellent biocompatibility and bioactivity. HAphas been extensively used in medicine for implant fabrication. It iscommonly the material of choice for the fabrication of dense and porousbioceramics. Its general uses include biocompatible phase-reinforcementin composites, coatings on metal implants and granular fill for directincorporation into human tissue. It has also been extensivelyinvestigated for non-medical applications such as a packingmaterial/support for column chromatography, gas sensors and catalysts,as a host material for lasers, and as a plant growth substrate. Allproperties of HAp, including bioactivity, biocompatibility, solubilityand adsorption properties can be tailored within a wide range bycontrolling qualitatively and quantitatively the ions substituted forCa²⁺, PO₄ ³⁻ and OH⁻ in the HAp lattice structure.

Magnesium has been known as one of the cationic substitutes for calciumin the HAp lattice structure. Magnesium-substituted HAp can be expressedby the simplified chemical formula:Ca_(10-x)Mg_(x)(PO₄)₆(OH)₂with x/10 representing atom-percent substitution of magnesium ions forcalcium ions.

Magnesium is also one of the predominant substitutes for calcium inbiological apatites. Enamel, dentin, and bone contain respectively 0.44wt %, 1.23 wt % and 0.72 wt % magnesium. Accordingly,magnesium-substituted HAp materials (Mg—HAp) are expected to haveexcellent biocompatibility and properties that can be favorably comparedwith those of hard tissue. U.S. Pat. No. 6,027,742 and WO 00/03747, forexample, disclose the use of Mg—HAp as bone substitutes and for dentalapplications, respectively.

Increasing concentration of MG in HAp has the following effects on itsproperties: (a) gradual decrease in crystallinity, (b) increase HPO₄incorporation, and (c) increase in extent of dissolution. Magnesium isclosely associated with mineralization of calcified tissues, andindirectly influences mineral metabolism. It has been suggested thatmagnesium directly stimulates osteoblast proliferation with an effectcomparable to that of insulin (a known growth factor for osteoblast).Thus, it becomes possible to tailor the physicochemical properties ofHAp, as well as its biocompatibility and bioactivity, by controlling theMg substitution of the HAp lattice structure.

Because the optimum amounts of magnesium in artificial HAp ceramics canvary with different applications, the capability to control preciselythe amounts of magnesium in HAp in the widest possible range bycontrolling the synthesis procedure is of primary importance. Mg—HAppowders have been prepared by precipitation and hydrolysis methods withthe replacement of calcium by magnesium limited to no more than 0.3 wt%.

Bigi et al., J. Inorg. Biochem, 49, 69-78(1993) disclosed the synthesisof crystalline Mg—HAp powders with up to about 30 atom-percent (about7.5 wt %) of magnesium under hydrothermal conditions at 120° C. Abovethis level of magnesium substitution the product was reported to becompletely amorphous. At most, 7 atom-percent (about 1.7 wt %) ofmagnesium ions were reported to be capable of substitution for calciumin the HAp lattice structure.

A need exists for crystalline Mg—HAp powders with a higher magnesiumcontent, a higher degree of magnesium-substitution in the HAp latticestructure, as well as a simple and inexpensive synthesis of Mg—HAp.

SUMMARY OF THE INVENTION

This need is met by the present invention. It has now been discoveredthat hybrid mechanochemical-hydrothermal synthesis techniques may beemployed to produce magnesium-substituted HAp with not only heretoforeunobtained magnesium levels, but also with levels of magnesiumincorporation into the HAp lattice structure that was not believedpossible until now.

Mechanochemical powder synthesis is a solid-state synthesis method thattakes advantage of the perturbation of surface-bonded species bypressure to enhance thermodynamic and kinetic reactions between solids.Pressure can be applied at room temperature by milling equipment rangingfrom low-energy ball mills to high-energy stirred mills. The mainadvantages of the mechanochemical synthesis of ceramic powders aresimplicity and low cost. Therefore, a variety of chemical compounds havebeen already prepared by this technique, for example CaSiO₃, PbTiO₃, and0.9Pb(Mg_(1/3)Nb_(2/3))O₃-0.1PbTiO₃, etc. Since the mechanochemicalsynthesis involves only solid-state reactions, it is clearlydistinguished from the mechanochemical-hydrothermal synthesis (sometimescalled “wet” mechanochemical), which takes advantage of the presence ofan aqueous solution in the system. An aqueous solution can activelyparticipate in the mechanochemical reaction by acceleration ofdissolution, diffusion, adsorption, reaction rate and crystallization(nucleation and growth). The mechanochemical activation of slurries cangenerate local zones of high temperatures (up to 450-700° C.) and highpressure due to friction effects and adiabatic heating of gas bubbles(if present in the slurry), while the overall temperature is close tothe room temperature.

The mechanochemical-hydrothermal technique is thus located at theintersection of hydrothermal and mechanochemical processing. Themechanochemical-hydrothermal route produces comparable amounts of HAppowder as the hydrothermal processing but it requires lower temperature,i.e., room temperature, as compared to typically 90-200° C. for thehydrothermal processing. Perhaps the biggest advantage of theroom-temperature mechanochemical-hydrothermal processing is that thereis no need for a pressure vessel and no need to heat the reactionmixture. The reaction is thus conducted either as a comminuting orstirred tank reaction process.

Therefore, according to one aspect of the present invention, a stable,phase-pure magnesium-substituted crystalline hydroxyapatite is providedcontaining from about 2.0 to about 29 wt % magnesium, wherein at least75 wt % of the magnesium content is substituted for calcium ions in thehydroxyapatite lattice structure. The Mg—HAp of the present inventionforms as crystal agglomerates. The present invention therefore alsoincludes particles of the Mg—HAp of the present invention having aparticle size between about 5 mm and about 100 microns.

The high magnesium content and high degree of magnesium substitution inthe HAp lattice structure is attributable to the combined use ofmechanochemical and hydrothermal process steps. Therefore, according toanother aspect of the present invention, a method for the preparation ofMg—HAp is provided, which includes the step of mechanochemicallyreacting in a stoichiometric ratio selected to provide a predeterminedlevel of magnesium substitution, a source of calcium ions, a source ofmagnesium ions, a source of phosphate ions and a source of hydroxideions, at least one of which is soluble in water, in an aqueous reactionmedium until Mg—HAp is formed. One material may serve as a multiple ionsource. For example, magnesium hydroxide may be employed as a source ofboth magnesium and hydroxide ions, or calcium hydrogen phosphate may beemployed as a source of calcium and phosphate ions.

The preferred source of phosphate ions is diammonium hydrogen phosphate,which is highly water soluble. Hydroxides of calcium and magnesium arepreferred sources of these two cations. With magnesium hydroxide, athigher levels of magnesium substitution, unreacted magnesium hydroxideshould be removed, preferably by washing the Mg—HAp in ammonium citrateaqueous solution so that the unreacted magnesium hydroxidepreferentially dissolves therein.

The ammonium citrate washing step represents a novel approach toincreasing the level of hydroxyapatite lattice-incorporated magnesiumrelative to the total magnesium content, as well as relative to thelattice-incorporated calcium. Therefore, according to another aspect ofthe present invention, a method is provided for increasing the magnesiumcontent in the lattice structure of magnesium-substituted crystallinehydroxyapatite relative to the calcium content of the lattice structureand to the non-lattice magnesium content, in which themagnesium-substituted hydroxyapatite is washed with an aqueous ammoniumcitrate solution.

The Mg—HAp of the present invention more closely resembles biologicalapatites than conventional HAp ceramics. Therefore, according to anotheraspect of the present invention there is provided a biocompatible hardtissue implant containing the Mg—HAp of the present invention. Forexample, metal or polymeric hard tissue implants may be created that arecoated with the Mg—HAp of the present invention, as well as implantsthat are formed from metal or polymeric Mg—HAp composite materials. Thepresent invention also includes a granular fill for direct incorporationinto human or animal tissues containing the Mg—HAp of the presentinvention, as well as dentifrice compositions, such as toothpaste, metalor polymeric composites for filling dental cavities, and bone cementscontaining the Mg—HAp of the present invention.

The easy to control stoichiometry makes the Mg—HAp of the presentinvention ideal for use as a packing material for chromatography columnsand gas sensors, as well as a support for catalytic materials or a plantgrowth substrate. Stoichiometric optimization can provide the end useproperties needed for each end-use application.

Therefore, accordingly to another aspect of the present invention, thereis provided a packing material for use in a chromatography column or gassensor, or as a support for a catalytic material, containing the Mg—HApof the present invention. The present invention also provides hostmaterials for luminescent applications containing the Mg—HAp of thepresent invention, as well as plant growth substrates containing theMg—HAp of the present invention.

The present invention thus provides a means by which levels of magnesiumsubstitution in HAp may be controlled by changing the ratio of calciumand magnesium ions in the source materials to tailor the end-product tospecific end-use applications. The foregoing and other objects,features, and advantages of the present invention are more readilyapparent from the detailed description of the preferred embodiments setforth below.

DETAILED DESCRIPTION OF THE PREFERRED EMBODIMENTS

The magnesium-substituted hydroxyapatites of the present invention areprepared by a combined mechanochemical-hydrothermal process. A source ofmagnesium ions, a source of calcium ions, a source of phosphate ions anda source of hydroxide ions are mechanochemically reacted in an aqueousreaction medium. At least one ion source is water-soluble.

For purposes of the present invention, “water-soluble” ion sources aredefined as being materials having a solubility in water of at leastabout 2.0 g/L. A solubility greater than about 20 g/L is preferred.

Examples of magnesium ion sources include magnesium hydroxide, magnesiumcarbonate, magnesium acetate, magnesium halides, magnesium oxide,magnesium nitrate, magnesium phosphate, and the like. Magnesiumhydroxide is preferred. Similarly, examples of calcium ion sourcesinclude calcium hydroxide, calcium carbonate, calcium acetate, calciumhalides, calcium oxide, calcium nitrate, calcium phosphate, and thelike. Calcium hydroxide is preferred.

Examples of phosphate ion sources include ammonium phosphates, calciumphosphates, magnesium phosphates, Group I phosphates such as potassiumand sodium phosphates, and the like. A water-soluble phosphate ionsource is preferred, with diammonium hydrogen phosphate beingparticularly preferred.

Hydroxide ion sources include hydroxide-containing compounds such asammonium hydroxide, calcium hydroxide, magnesium hydroxide, sodiumhydroxide, potassium hydroxide, and the like, and compounds thatgenerate hydroxide ion in aqueous solution, such as ammonia, calciumoxide, magnesium oxide, and the like.

Depending upon the end-use application, other ion sources may beincluded as well, of a quality and quantity that do not disrupt thehydroxyapatite lattice structure. Thus, quantities of source materialsmay be employed that introduce up to about 25 wt % into the Mg—HAplattice structure, depending upon the ions, of one or more cations, forexample, sodium, lithium, barium, strontium, zinc, cadmium, lead,vanadium, silicon, germanium, iron, arsenic, manganese, aluminum, rareearth elements, cobalt, silver, chromium, antimony, and the like, or oneor more anions, for example, carbonate, halides, oxygen, sulfur and thelike. Suitable additional ion sources and appropriate quantities thereofare readily determined by those of ordinary skill in the art withoutundue experimentation.

Preferably, at least one ion source is water-insoluble or reacts to forman insoluble apatite phase precursor. This provides a substrate mediumfor the application of mechanochemical force at the same time that thehydrothermal process steps are being carried out.

Stoichiometric quantities of the ion sources are employed, selected toprovide the desired ratio of individual HAp lattice components,especially the ratio of calcium to magnesium and the ration cationsoccupying the calcium sites to phosphorous. Water-soluble ion sourcesare dissolved in the aqueous reaction medium, with a slurry being formedof the non-water-soluble ion sources. The preferred aqueous medium isessentially pure distilled water, that more preferably has beendeionized and/or demineralized. Up to about 40 wt % of the combinedamounts of the ion sources may be added to the aqueous reaction medium,at a temperature maintained between about 8 and 35° C., and preferablybetween about 25 and about 35° C., until Mg—HAp is formed. Externalsources of heat are not needed, with sufficient heat being supplied bymilling friction. Instead, external cooling may be needed because themolecular activation of the slurry can generate local zones of hightemperature (up to 450-700° C.) and corresponding pressures due tofriction and adiabatic heating of gas bubbles.

With stirring of the aqueous slurry/solution, the ion sources aremechanochemically reacted, typically by the application of physicalforce to the water-insoluble ion sources or insoluble apatite precursorsthat are suspended as a slurry in the aqueous reaction medium containingthe water-soluble ion sources. Preferred mechanochemical reactionprocesses comminute the ion source slurry particles, preferably bymilling or grinding the water insoluble ion source particles withheating of the aqueous reaction medium into which the water-soluble ionsource has been dissolved. Preferred methods at the same timefrictionally heat the aqueous reaction medium/slurry while the slurryparticles are being milled or ground, so that the mechanochemical andhydrothermal process step are performed simultaneously.

Multi-ring media mills are preferred. The grinding mechanism consists ofa central rotating stainless steel shaft, which drives a plurality ofstainless steel sub-shafts (sleeve-lined with zirconia-toughenedalumina) that are connected symmetrically to the central shaft. Eachsub-shaft contains a plurality of stacked zirconia rings, which rotateeccentrically around each sub-shaft. When the central shaft is rotating,the zirconia rings on the sub-shafts are moved by the centrifugal forceradially outwards, applying force on the inner wall of the millingvessel, which is ceramic lined. Solid slurry particles located betweenthe rotating rings and the liner wall are consequently comminuted.

The comminuting step is performed at rotation speeds between 800 and1500 r.p.m. (for the multi-ring media mill), or higher for higher solidcontent slurries for at least 1 hour, and preferably from between about1 and about 10 hours, with the temperature of the aqueous slurrymaintained between about 25 and about 35° C. for the duration. The solidphase is then recovered and washed with distilled water, preferablyrepeatedly. The solid phase is then once again isolated and excess wateris removed, preferably by first centrifuging the material followed byoven drying at a temperature between about 40 and 200° C. Lyophilizationmay also be employed to remove excess water. If desired, dry grindingmay be performed to reduce the powder particle size.

The inventive method advantageously employs environmentally benign ionsources in an aqueous reaction medium at mild temperatures. The elevatedtemperatures associated with prior art calcination processes are therebyavoided.

When all of the ion sources are water-soluble a solution-phase reactionis first performed, followed by heating to drive off the aqueous phaseto recover a powder material that is milled while wet through to drynessto complete the mechanochemical reaction. However, a slurry-basedreaction is preferred in which one of the ion sources iswater-insoluble. Or two water-soluble material may be employed that forman insoluble apatite precursor that is then milled while wet through todryness to complete the mechanochemical reaction. Under certaincircumstances understood by those skilled in the art, Mg—HAp's ofpresent invention may be produced solely by dry milling.

With water-insoluble magnesium ion sources, such as magnesium hydroxide,magnesium oxide, magnesium phosphates, and the like, for higher levelsof magnesium substitution, unreacted quantities of the magnesium ionsource will remain that have to be removed by selective washing of theMg—HAp. In a particularly preferred embodiment, the Mg—HAp is washedwith ammonium citrate aqueous solution, into which the unreactedmagnesium ion source will preferentially dissolve. After this washingstep, the purified Mg—HAp is washed, preferably repeatedly, withdistilled water and then dried.

In a preferred procedure Mg—HAp powders are prepared by suspending amixture of calcium hydroxide and magnesium hydroxide powders in waterand subsequently adding a soluble diammonium hydrogen phosphate powder,quantities as required by stoichiometry. Themechanochemical-hydrothermal synthesis is then performed by placing theslurry into a multi-ring media mill and then grinding the slurry. Theresulting powder is washed using water to remove soluble salts with anammonium citrate aqueous solution washing step performed first forreactions employing higher levels of magnesium substitution. Followingthe water washing, the Mg—HAp is then dried.

The inventive method provides crystalline Mg—HAp powders in which atleast 75 wt % of the magnesium content is substituted for calcium ionsin the hydroxyapatite lattice structure. Crystalline Mg—HAp in whichessentially all of the magnesium content is substituted for calcium ionsin the hydroxyapatite lattice structure can be readily obtained withoutundue effort. Accordingly, substitution levels between about 80 wt % and98 wt % can be readily obtained by the ordinarily skilled artisanfollowing the teachings of the present specification.

The crystalline Mg—HAp will have a magnesium content between about 2.0and about 29 wt %, with levels between about 3.5 and about 28.4 wt %being preferred. Levels between about 5 and about 25 wt % are even morepreferred, with a level of at least 10 wt % being most preferred. Thecrystalline Mg—HAp of the present invention forms crystals agglomerateshaving an approximate particles ranging in size between about 5 nm andabout 10 microns.

The crystalline Mg—HAp of the present invention is useful in thepreparation of compounds for use as granular fill for directincorporation into the hard tissues of humans or other animals, and asbone implantable materials. The present invention thus includes granularfill compounds, bone implant materials, tooth filling compounds, bonecements and dentifrices containing the Mg—HAp of the present invention.The products are formulated and prepared by substituting the Mg—HAp ofthe present invention for HAp in conventional HAp-based products. Thecompounds may be prepared from metallic and polymeric Mg—HAp composites.

The Mg—HAp of the present invention may also be substituted for the HApin support materials for gas sensors and chromatography columns. It mayalso be substituted for HAp and other support substrates and hosts incatalytic supports, plant growth substrates and in host materials forluminescent applications. Therefore, the present invention also includespacking materials for chromatography columns and gas sensors, catalyticsupports, plant growth substrates and host materials for luminescentapplications containing the Mg—HAp of the present invention.

The following non-limiting examples set forth herein below illustratescertain aspects of the invention. All parts and percentages are byweight unless otherwise noted and all temperatures are in degreesCelsius. Stoichiometric values in HAp and Mg—HAp formulas areapproximate.

EXAMPLES Example 1 Mechanochemical-Hydrothermal Synthesis ofCa₈Mg₂(PO₄)₆(OH)₂

Calcium hydroxide, magnesium hydroxide and solid diammonium hydrogenphosphate (analytical grade, Alfa Aesar, Ward Hill, Mass.) were used asreactants for the synthesis of Mg—HAp. First, a suspension containing apowder mixture of 22.170 g calcium hydroxide and 4.557 g magnesiumhydroxide in 350 mL deionized water was prepared inside a 500 ml glassbeaker. Subsequently, 29.410 g of diammonium hydrogen phosphate powderwas slowly added to the same beaker at constant vigorous stirring usinga magnetic stirrer for about 10 minutes. The (Ca+Mg)P molar ratio in thestarting slurry was 1.67. The presence of water adsorbed on allreactants was measured by thermogravimetry to maintain the targetedstoichiometry. The pH of the slurry was about 10.3, measured using aglass electrode connected to a small pH-meter (ACCUMET™ Model 805 MP,Fisher Scientific, Pittsburgh, Pa.) and calibrated with respect to abuffer solution (pH=10.00, Fisher Scientific). Themechanochemical-hydrothermal synthesis was performed by placing theslurry into a laboratory scale mill (Model MIC-0, NARA Machinery Co.,Tokyo, Japan) equipped with a zirconia liner and a zirconia ringgrinding media. Grinding of the slurry was carried out in air, initiallyat a rotation speed of 1500 rpm for one hour and then at 800 rpm forfour hours. Temperature during the grinding was measured using athermocouple and determined to be 33° C. at 1500 rpm and 28° C. at 800rpm.

Washing of the solid phase after the mechanochemical-hydrothermalsynthesis was accomplished by four cycles of shaking the solid withdistilled water in 250 mL HDPE bottles using a hand shaker machine ModelM37615, Barnstead/Thermolyne, Dubuque, Iowa) followed by centrifuging at4500 rpm for 30 minutes (Induction Drive Centrifuge, Model J2-21M,Beckman Instruments, Fullerton, Calif.). The washed solid phase wasdried in an oven at 70° C. for 24 hours (ISOTEMP™ Oven, Model 230GFisher Scientific) and ground into powder.

The synthesized Mg—HAp powder contained a fraction of unreactedmagnesium hydroxide. Therefore, it was suspended in a 0.2 M ammoniumcitrate aqueous solution. The ammonium citrate solution was prepared ina 200 mL glass beaker by dissolving 3.843 g of solid citric acid(reagent grade, Aldrich, Milwaukee, Wis.) in 100 mL of distilled waterand subsequently slowly adding ammonia solution (reagent grade, FisherScientific) to yield a pH between 8 and 10. 1.0 g of the Mg—HApcontaining unreacted magnesium hydroxide was then suspended in thesolution. The dissolution of the magnesium hydroxide was accomplishedunder a vigorous stirring using a magnetic stirrer for 12 hours, afterwhich the prior distilled water washing, centrifuging and drying stepswere repeated.

Phase pure crystalline Mg—HAp essentially free of unreacted magnesiumhydroxide and having a magnesium content of approximately 10 wt % inwhich essentially all of the magnesium content was substituted forcalcium ions in the hydroxyapatite lattice structure was confirmed byx-ray defraction, Fourier Transform Infra-Red spectroscopy,thermogravimetric analysis and chemical analysis.

Dynamic light scattering revealed the particle size distribution of theMg—HAp to be between about 130 and about 2100 nm with a specific surfacearea of about 129 m²/g, indicating agglomeration. Scanning ElectronMicroscopy confirmed agglomerates of nanosized Mg—HAp crystals.

Example 2 Mechanochemical-Hydrothermal Synthesis of Ca₇Mg₃(PO₄)₆(OH)₂

Ca(OH), MG(OH)₂ and solid (NH₄)₂HPO₄ (analytical grade, Alfa Aesar, WardHill, Mass.) were used as reactants for the synthesis of Mg—HAp. First,a suspension containing a powdered mixture of 19.150 g Ca(OH)₂ and 6.717g Mg(OH)₂ in 350 mL of deionized water was prepared inside a 500 mLglass beaker. Subsequently, 29.028 g of (NH₄)₂HPO₄ powder was slowlyadded to the same beaker at constant vigorous stirring using a magneticstirrer for about 10 min. The (Ca+Mg)/P molar ratio in the startingslurry was 1.67. The presence of water adsorbed on all reactants wasmeasured by thermogravimetry to maintain the targeted stoichiometries.The pH of the slurry was about 10.2, measured using a glass electrodeconnected to a pH-meter (Accumet Model 805 MP, Fisher Scientific,Pittsburgh, Pa.) and calibrated with respect to a buffer solution(pH=10.00, Fisher Scientific).

The mechanochemical-hydrothermal synthesis was performed by placing theslurry into a laboratory-scale mill (model MIC-0, NARA Machinery Co.,Tokyo, Japan) equipped with a zirconia liner and zirconia ring grindingmedia. Grinding of the slurry was carried out in air, initially at arotation speed of 1500 rpm for 1 h and then at 800 rpm for 4 h.Temperature during the grinding was measured using a thermocouple andwas determined to be 33° C. at 1500 rpm and 28° C. at 800 rpm. Washingof the solid phase after the mechanochemical-hydrothermal synthesis wasaccomplished by 2-6 cycles of shaking the solid with distilled water in2-6 HDPE 250 mL bottles using a hand shaker machine (Model M37615,Barnstead/Thermolyne, Dubuque, Iowa) followed by centrifuging at 4500rpm for 30 min. (Induction Drive Centrifuge, Model J2-21M, BeckmanInstruments, Fullerton Calif.).

The washed solid phase was dried in an oven at 70° C. for 24 h (Isotempoven, model 230G, Fisher Scientific) and ground into powder. Thesynthesized MG-HAp powder contained a fraction of unreacted Mg(OH)2.Therefore, it was suspended in 0.2 M-ammonium citrate aqueous solution.The ammonium citrate solution was prepared in a 250 mL glass beaker bydissolving 3.843 g of solid citric acid (reagent grade, Aldrich,Milwaukee, Wis.) in 200 mL of distilled water and subsequently slowlyadding ammonia solution (reagent grade, Fisher Scientific) to yield a pHof 10. 1.0 g of the Mg—HAp containing unreached Mg(OH)₂ was thensuspended in the solution. The dissolution of the Mg(OH)₂ wasaccomplished under a vigorous stirring using a magnetic stirrer for 24h. This procedure was repeated once under the same conditions, in orderto completely remove the Mg(OH)₂ phase.

Properties: Mg content: 15 wt %, particle size distribution: 250-4500nm, SSA: 115 m²/g.

Comparative Example

Example 1 was repeated substituting 2-propanol (C₃H₇OH, histologicalgrade, Fisher Scientific) for water, so that the reaction conditionswere purely mechanochemical. Under otherwise equivalent conditions, noMg—HAp was observed to form. This emphasizes the importance of thehydrothermal conditions provided by the aqueous reaction medium in whichat least one of the ion sources is soluble, and which thus activelyparticipates in the synthesis reaction by dissolving one of thereactants.

The present invention thus provides for the reproducible and low-costfabrication of high-quality Mg—HAp powders in large batch sizes. Theforegoing examples and description of the preferred embodiment should betaken as illustrating, rather than as limiting the present invention asdefined by the claims. As will be readily appreciated, numerousvariations and combinations of the features set forth above can beutilized without departing from the present invention as set forth inthe claims. Such variations are not regarded as a departure from thespirit and scope of the invention, and all such variations are intendedto be included within the scope of the following claims.

1. A stable, phase-pure magnesium-substituted crystalline hydroxyapatitecomprising from about 2.0 to about 29 wt % magnesium, wherein at least75 wt % of the magnesium content is substituted for calcium ions in thehydroxyapatite lattice structure.
 2. The phase-puremagnesium-substituted crystalline hydroxyapatite of claim 1, comprisingfrom about 3.5 to about 28.4 wt % magnesium.
 3. The phase-puremagnesium-substituted crystalline hydroxyapatite of claim 2, comprisingfrom about 5 to about 25 wt % magnesium.
 4. The phase-puremagnesium-substituted crystalline hydroxyapatite of claim 1, whereinessentially all of the magnesium content is substituted for calcium ionsin the hydroxyapatite lattice structure.
 5. The phase-puremagnesium-substituted crystalline hydroxyapatite of claim 1, comprisingcrystal agglomerates having a particle size between about 5 nm and about100 microns.
 6. A packing material for use in a chromatography column orgas sensor or as a catalytic support comprising themagnesium-substituted hydroxyapatite of claim
 1. 7. A biocompatible hardtissue implant comprising the magnesium-substituted hydroxyapatite ofclaim
 1. 8. The biocompatible hard tissue implant of claim 7, comprisinga metal or polymeric implant coated with said magnesium-substitutedhydroxyapatite.
 9. The biocompatible hard tissue implant of claim 7,comprising a polymeric composite.
 10. A granular fill for directincorporation into human or animal tissues comprising themagnesium-substituted hydroxyapatite of claim
 1. 11. The granular fillof claim 10, comprising a metal or polymeric composite for fillingdental cavities.
 12. A plant growth substrate comprising themagnesium-substituted hydroxyapatite of claim
 1. 13. A dentifricecomposition comprising the magnesium-substituted hydroxyapatite ofclaim
 1. 14. A host material for luminescent applications comprising themagnesium-substituted hydroxyapatite of claim 1.